Welcome to your personal class wiki page. Only you should edit this wiki and no other page unless designated by Mr. Miller. It is very important that you follow this protocol. If you edit another student's page it will show in the history of that page and you will be penalized or reprimanded appropriately. This should be a fun activity and will be part of your grade. If you have any questions feel free to email Mr. Miller at any time. Parts of the earth assignment
What is the main composition of the Earth's core? Nickel and Iron
Which layer of the Earth is thinnest? Crust
Which layer of the Earth is the source of all of the materials that we use? Mantle Crust
What is the theory that describes the changes of the earth's surface over time? plate tectonics theory
Which layer of the Earth is described in question 4? The earth's outer layerCrust
Which type of boundary marks the location where two plates move apart from one another? Divergent boundary
Give an example of a transform boundary.. The boundary between the Pacific Plate and the Australian Plate, crossing New Zealand.
Define a subduction zone. the place where two lithospheric plates come together, one riding over the other.
What causes sea floor spreading? Divergent boundaries in the middle of the ocean
Describe the formation of a rift. When two continental plates diverge, a valleylike rift develops.
Mineral assignment
Identify the 5 essential characteristics of a mineral.
It must occur naturally.
It must be inorganic It must be a solid It must possess an orderly internal structure, that is, its atoms must be arranged in a definite pattern. It must have a definite chemical composition that may vary within specified limits."
Identify three properties used to identify minerals. hardness, optical properties, crystal structure.
Identify three examples a mineral. Identify the composition of each mineral by the formula of the compound and name of a compound. Mircocline is a silicate of potassium and Al2SiO4 (F,OH)2aluminum;KAlSi3O8 . Talc is a silicate of magnesium;Mg3Si3O10(OH)3 . Topaz is a silicate of aluminum Al2SiO4 (F,OH)2
Converting Copper Wednesday, January 26, 2011 9:57 AM
Mass
Crucible alone
4.06g
Lid alone
3.67g
Crucible + lid
7.73g
Crucible + copper
5.08g
Crucible +lid + copper
8.73g
Copper powder before heating
1.02g
beginning Observation Shiny, metallic Small tiny pieces
mass
Crucible+ copper+ lid
8.74g
Crucible + copper
5.06g
Copper alone
3.68g
(Based upon your data, it would appear that the mass decreased by 0.02g. This may be due to human or mechanical error.)
After observation grey & dull Small tiny pieces Ia.physical (-2) b.Because the copper's color changed from shiny ! metallic copper how its grey 2a. When the lid was taken off the copper turned Into rainbow then back to a grey b. Yes because more mass was added, so nothing left the crucible. 3.a. the mass went up b. oxygen.(What does this mean? -1)
Metal Reactivity Assignment
Describe what happens to the penny when it is placed in the sliver nitrate solution. The shiny reflective surface of the coin immediately turns dark.
Describe how ions in solution play a role in chemical reactivity. They gain electrons causing the reaction
Explain, in detail, why this is happening. The copper surface silver ions gain one electron each to become silver atoms and since they're now neutral they stay on the surface.
Define Oxidation. Atoms leaving its two electrons in the metal structure
Define Reduction. Ions gaining an electron from one of the copper atoms.
Explain what happens to the copper atoms during the redox reaction. Every two electrons lost by a copper atom,two silver ions gain one electron each.
Explain what happens to the silver ions during the redox reaction. Silver electrons pulls away from the copper atoms.
What ultimately controls chemical reactivity? The collision of two compounds in a orientation
RELATIVE REACTIVITIES OF METALS LAB Friday, January 28, 2011 9:47 AM
CuNO3
AgNO3
MgNO3
ZnNO3
Cu
No reaction
Turned the copper black
no reaction
No reaction
Mg
Turned black. Looks like it was burned
Turned black
No reaction
Made it more shiny
Zn
Turned black
Turned black
No reaction
no reaction
Ag
No reaction
NO reaction
No reaction
No reaction
Lab Questions 1. Which metal reacted with the most solutions? Magnesium
2. Which metal reacted with the fewest solutions? Silver
3. With which of the solutions (if any) would you expect silver metal to react, if it were available to be tested? None Any metals less reactive than silver.
4. List the metals (including silver) in order, placing the most reactive metal first (the one reacting with the most solutions) and the least reactive metal last (the one reacting with the fewest solutions). Mg,Zn,Cu,Ag.
5. Refer to your “metal activity series” list in Question 4. Write a brief explanation of why the outside surface of a penny is made of copper instead of zinc. The outside of a penny is made from copper instead of zinc because copper is less reactive than zinc and unlike zinc copper coins wont react in your pocket.
6. a. Which of the four metals mentioned in this laboratory activity might be an even better choice than copper for the outside. surface of a penny? Why? Silver because it didn't react with any of the solutions b. Why do you think that metal is not used for that purpose? Silver isn't used because it's a expensive material and it would cost more to make the coin than the silver.
7. Given your new knowledge about the relative chemical activities of these four metals, a. which metal is most likely to be found in an uncombined, or “free,” (metallic) state in nature? Ag because it wouldn't react with anything and just stay in it original state. b. which metal is least likely to be found chemically uncombined with other elements? Magnesium because its been proven to be highly reactive.
8. Reconsider your experimental design for this activity. a. Would it have been possible to eliminate one or more of the metal-solution combinations and still obtain all information needed to create chemical activity ratings for the metals? Yes b. If so, which combination(s) could have been eliminated? Why? MgNO3 could of been eliminated because it didn't react with any of the metals.
Activity Series of Metals Assignment (Oxidation/Reduction Part I)
1) a. Magnesium is surrounded by a two-electron cloud. It gets smaller b. Zinc is surrounded by a two-electron cloud. c. Zn2+ ions rise to the top of the Magnesium gaining two electrons each becoming Zinc atoms. d. When Mg2+ ions rises to the surface of the Zinc there's no reaction.
2) a. Mg2+ + copper --> No reaction b. Zn2+ + copper--> No reaction c. Cu2+ + Mg --> Cu2+ ions gain 2 electrons each becoming Copper atoms d. Cu2+ + Zn --> Cu2+ ions gain 2 electrons each becoming Copper atoms
3) a. Ag+ & Magnesium reactive. Mg+ ions gain an electron each becoming Magnesium atoms. b. Ag+ & Zinc reactive. Ag+ ions gain an electron each becoming Magnesium atoms c. Zn2+ & Silver are non reactive. d. Mg2+ & Silver are non reactive.
4) Magnesium, Zinc, Copper, Silver
ChemQuandry 1/Building Skills 5
1) Copper, gold, and silver are far from being the most abundant metals on Earth. Aluminum, iron, and calcium, for example, are all much more plentiful. Why, then, were copper, gold, and silver among the first metallic elements discovered? Because they are highly prized in long-lasting, decorative objects and they don't react with things in nature or other chemicals.
Building Skills 5
Use the table in Figure 16 and the Periodic Table (page 104) to answer the following questions.
1. a. What trend in metallic reactivity is found from left to right across a horizontal row (period) of the Periodic Table? (Hint: Compare the reactivities of sodium, magnesium, and aluminum.) The reactivity of the elements decreases as it moves from left to right on the periodic table. b. In which part of the Periodic Table are the most-reactive metals found? Alkali metal c. Which part of the Periodic Table contains the least-reactive metals? right side of Transition Metals
2. a. Will iron (Fe) metal react with a solution of lead(II) nitrate, Pb(NO3)2? Yes b. Will platinum (Pt) metal react with a lead(II) nitrate solution? Yes c. Explain your answers to Questions 2a and 2b. If the solution is a higher has a reactivity than the metal then nothing will happen but if the metal has a higher reactivity than the solution its going to react.
3. Use specific examples from the activity series in your answers to these two questions: a. Are least-reactive metals also the cheapest metals? No b. If not, what other factor(s) might influence the market value of a metal? They are long lasting and they don’t react with oxygen. supply and demand
MODELING MATTER
1. Construct a similar electron-dot expression for the change that occurred in Laboratory Activity B.4 when each of these events took place: a. An atom of zinc, Zn, was converted to a Zn2 ion. (Hint: Zn has two readily removable electrons.) Zn: --> Zn2+ + 2e- oxidation b. A silver ion, Ag+ was converted to a metallic silver atom, Ag(s). Ag+ + e- -----> Ag. reduction
2. Apply the definitions of oxidation and reduction to your two equations in Question 1.
3. a. Which reactant (Cu or Ag) is oxidized? copper b. Which is reduced? Ag+
4. Why are two Ag+ ions needed for each Cu(s) atom that reacts? Because copper loses two electrons each and the copper atoms are oxidized,so the two electrons are then replaced by the two Ag+ ions.
5. a. Given that definition and explanation, what must be the reducing agent in the reaction between Cu(s) and Ag+ ions? Copper b. How would you define a reducing agent? The atoms in the reaction loses electrons.
6. Draw an electron-dot representation of this reaction. Zn2+(s) + Cu(aq) ----> Zn2+ (aq) + Cu(s)
7.Which is the oxidized? a.Cu2+ (aq) b. Which is the reducing? Zinc
8. Cu2+ (aq) is the oxidizing agent and the zinc is the reducing agent.
9. You could tell by the more reactive element. The most reactive element would be the oxidizing agent and the less reactive one would be the reducing agent.
10.a.The oxidized isZn2+(aq) b.The reduced is Mg(s) c.The oxidizing agent is Zn2+(aq) d.The reducing agent is Mg(s)
RETRIEVING COPPER LAB
1st mass
2nd mass
Filter paper
0.70 g
0.71g
Filter+ copper
1.67g
0.81g
solid copper
0.97g
0.1g
Observations
•the black copper turned copper color again HCL turned yellow -The zinc reacted right away when it was put in the HCL - bubbled;fizzed
Questions
1.
In Laboratory Activity B.2 not all of the original copper powder reacted when you heated it in air. a. Why do you think the reaction was incomplete? pentine b. How would you revise the procedure so that more copper(II) oxide could form? Heat it more. Clean them with sandpaper or steel wool.(damage the surface)
2. a. In Laboratory Activity B.2 what mass of the original copper powder sample reacted when you heated it? (Hint: Use the original mass of copper used in Laboratory Activity B.2 and the mass of copper residue found in Step 8 to calculate this.) .3g of copper powder b. What percent of the total copper-powder sample reacted? 30%
3. In the reaction between copper(II) chloride (CuCl2) solution and zinc metal, each Cu2 ion gained two electrons to form an atom of
copper metal. Each zinc metal atom lost two electrons to form a Zn2 ion.
a. Write a chemical equation that represents this process. (To review how, turn to pages 122–123.) Zn(s) + Cu2+(aq) ---> Zn2+ (aq) + Cu(s) b. Based on the equation you wrote in Question 3a, identify i. the species that was oxidized. Zinc ii. the species that was reduced. copper iii. the reducing agent. copper iv. the oxidizing agent. Zinc
4. Adding HCl to CuO resulted in the formation of a blue solution. Thiscolor is due to the presence of Cu2(aq) ions. Consult your observations in answering these questions: a. Describe what happened to the solution color after you added zinc in Step 9. The color got brighter and clearer. b. What caused the changes you observed in the solution? the zinc ions went into the solution. c. How can the color of the solution be used to indicate when the zinc metal has removed the Cu2 ions in solution? If the solution has changed from the blue color to the light clear blueish color then you know the zinc metal has been removed.
5. To recover Cu metal from the CuCl2 solution, you had to use other resources. a. What resources were “used up” in this process?Zinc and HCL
b. Where did each of them go?
READING QUESTIONNAIRE
1.Describe the main differences between renewable and nonrenewable resources and provide an example of each. Renewable resources can be replenished and a nonrewable resource can't be replenished. An example for a renewable resource air and an example for nonrenewable resource is natural gas.
2. a) If atoms are always conserved why do some people say that a resource may be “running out”?
b) Can a resource actually “run out”?
3.) What are the requirements for minimum profitability levels for a metal in an ore? As low as 1% for copper or 0.001% for gold to as high as 30% of aluminum.
4.) Identify and explain the two strategies for avoiding the depletion of metal ores.
Slowing down the rate of the use of resources.
Replace a resource by finding substitute materials with similar properties.
5.) Can recycling also create environmental problems? If so, explain how this can happen. Yes because aluminum scaps may contain up to 1% of magnesium and to properly remove the magnesium they would have to use chlorine gas which can lead to air pollution.
6.) How much trash does the average person produce per day? 4lbs a day.
7.) Identify two ways that consumer products can become waste. telephones and yesterday's newpaper.
8.)Describe a way of dealing with recyclable waste that might be profitable good for energy use. combustion for energy. ( waste-to-energy)
9.)What are the three options for the final step in the life cycle of a material? Recycle,Landfills, and combustion for energy.
10.) Which waste category has the greatest weight before recycling? What is the weight of this waste produced? Paper, 83.8 million tons.
11.) Using Figure 21 on page147 identify which waste category has the least weight before recycling? What is the weight of this waste? Wood, 11.6 million tons
12.)Calculate the difference between the waste produced from your answer to question 11 and the amount of waste produced after recycling. Remember these values are in millions of tons, so make sure that you calculate correctly and label with the correct units of measure. (1 ton = 2000 lbs) .6million tons
13.)If we compare the Total Generation of Waste (before recycling) to the Total Discards of Waste (after recycling), what percentage of waste is actually thrown away? What percentage of the Total Generation of Waste is actually recycled? Show your calculations below using the correct units of measure and labels. 72% of actual waste is thrown away. 28% total generation of waste is actually recycled
14.) Draw the diagram in Figure 22, on page 148, in the space below. Compare this to Figure 20 on page 146. Match and Label the location of the steps in figure 20 to your diagram by connecting them with lines/arrows around the outside. will show you in class
BUILDING SKILLS 11
1)
STRIKING IT RICH LAB
Observations -when the pennies were dropped into the Zn and ZnCl2 solution it then dark grey then when dropped into the water it turned silver like a nickel. - the pennies were put into the flame then dropped into water the pennies started to take on a gold color.
Condition
Appearance
Untreated penny
shiny,round,bronze
Penny treated with Zn and ZnCl2
grey, bubbled a bit,silver like a nickel
Penny treated with Zn and ZnCl2 and
heated in burner flame
gold with some silver,shiny
LAB QUESTIONS
1) a. The untreated penny is a copper/bronze color,look like a ordinary penny. The penny treated with the Zn and ZnCl2 has a silver coating and the penny with Zn and ZnCl2 and heated in the burner flame has a gold coating.
b. Yes the penny treated with Zn and ZnCl2 is composed of Copper and Zinc and the penny treated with Zn and ZnCl2 and the burner is composed of Zinc and Copper. (True, but what does the penny "look" like? Does it appear to be "gold" or "silver"?) -1
2) Their claim would be incorrect because the penny is made of copper and it just has a coating on of zinc on it. (Prove it. What does the Law of Conservation of Matter say?) -2
3) Pipes and bridges (Pipes maybe but bridges? This type of process is more for coating common materials like jewelry or something smaller.) -1
4) a. The copper atoms went into the solution.(No the copper atoms stayed right where they were, in the penny.) -2
b. Yes. The same procedure from the Retrieving copper activity would have to be done in order to convert the pennies back to its copper state. (You could do that. Good answer.)
BUILDING SKILLS 12
1) Pluming(pipes) - Lead
Electrical wiring- silver
Pot and pans- iron
shell casing- silver
2) magnesium,potassium,lithium,
3) shell casings and electrical wiring because its would last longer.
SECTION 3.A
HYDROCARBON BOILING POINTS
1) A. Its organized in alphabetical order.
B.Yes because it can help people remember the names and the boiling points.
2) A. Lowest to highest boiling point.
B.
Methane
-161.7
Ethane
-88.6
Propane
-42.1
Butane
-0.5
Pentane
36.1
Hexane
68.7
Heptane
98.4
Octane
125.7
Nonane
150.8
Decane
174.0
3) Butane,Propane,Ethane,Methane
4) Petane
5) The intermolecular forces in Decane are more active than those in Butane.
SEPARATION BY DISTILLATION LAB QUESTIONS(30/42)
2) A. 86degrees C; 95 degrees C
3) Distillation 1 was Acetone and Distillation2 was Propanol. (D-1 = propanol, D-2 = water -2)
4) Didn't get information. (-2)
5) Distillation 2 because it reacted with iodine better than distillation 1.
6) By looking at the appearance or test samples of the solution against other substances. (explain? -1)
7) Cyclohexane and water because it is a long and drawn out process that takes to much energy. (What about propanol? Isn't the boiling point closest to cyclohexane? -1)
8) ? (-6)
BUILDING SKILLS 3
1) The more the carbon-chain branches increases the higher the boiling point because there is more energy needed to move the atoms around.
a. 98.4 degreesC
b. 92.0 degreesC
c. 79.2 degreesC
3)
a. The figure would have a lower BP than the single chain and the one branch chain. It would also have a higher BP than the three branch.
b. Higher
4.) The parent chain determines the boiling point, so the longer the parent chain the boiling point.The straighter the chain the higher the BP and the more it branches out the lower the BP will be.
Parts of the earth assignment
Mineral assignment
- Identify the 5 essential characteristics of a mineral.
It must occur naturally.It must be inorganic
It must be a solid
It must possess an orderly internal structure, that is, its atoms must be arranged in a definite pattern.
It must have a definite chemical composition that may vary within specified limits."
Converting Copper
Wednesday, January 26, 2011
9:57 AM
beginning Observation
Shiny, metallic
Small tiny pieces
After observation
grey & dull
Small tiny pieces
Ia.physical (-2)
b.Because the copper's color changed from shiny ! metallic copper how its grey
2a. When the lid was taken
off the copper turned Into rainbow then back to a grey
b. Yes because more mass was
added, so nothing left the crucible.
3.a. the mass went up
b. oxygen. (What does this mean? -1)
Metal Reactivity Assignment
RELATIVE REACTIVITIES OF METALS LAB
Friday, January 28, 2011
9:47 AM
Lab Questions
1. Which metal reacted with the most solutions? Magnesium
2. Which metal reacted with the fewest solutions? Silver
3. With which of the solutions (if any) would you expect silver metal to
react, if it were available to be tested? None Any metals less reactive than silver.
4. List the metals (including silver) in order, placing the most reactive
metal first (the one reacting with the most solutions) and the least
reactive metal last (the one reacting with the fewest solutions). Mg,Zn,Cu,Ag.
5. Refer to your “metal activity series” list in Question 4. Write a brief
explanation of why the outside surface of a penny is made of copper
instead of zinc.
The outside of a penny is made from copper instead of zinc because copper is less reactive than zinc and unlike zinc copper coins wont react in your pocket.
6. a. Which of the four metals mentioned in this laboratory activity
might be an even better choice than copper for the outside.
surface of a penny? Why? Silver because it didn't react with any of the solutions
b. Why do you think that metal is not used for that purpose? Silver isn't used because it's a expensive material and it would cost more to make the coin than the silver.
7. Given your new knowledge about the relative chemical activities of
these four metals,
a. which metal is most likely to be found in an uncombined, or
“free,” (metallic) state in nature? Ag because it wouldn't react with anything and just stay in it original state.
b. which metal is least likely to be found chemically uncombined
with other elements? Magnesium because its been proven to be highly reactive.
8. Reconsider your experimental design for this activity.
a. Would it have been possible to eliminate one or more of the
metal-solution combinations and still obtain all information
needed to create chemical activity ratings for the metals? Yes
b. If so, which combination(s) could have been eliminated? Why? MgNO3 could of been eliminated because it didn't react with any of the metals.
Activity Series of Metals Assignment (Oxidation/Reduction Part I)
1) a. Magnesium is surrounded by a two-electron cloud. It gets smaller
b. Zinc is surrounded by a two-electron cloud.
c. Zn2+ ions rise to the top of the Magnesium gaining two electrons each becoming Zinc atoms.
d. When Mg2+ ions rises to the surface of the Zinc there's no reaction.
2) a. Mg2+ + copper --> No reaction
b. Zn2+ + copper--> No reaction
c. Cu2+ + Mg --> Cu2+ ions gain 2 electrons each becoming Copper atoms
d. Cu2+ + Zn --> Cu2+ ions gain 2 electrons each becoming Copper atoms
3) a. Ag+ & Magnesium reactive. Mg+ ions gain an electron each becoming Magnesium atoms.
b. Ag+ & Zinc reactive. Ag+ ions gain an electron each becoming Magnesium atoms
c. Zn2+ & Silver are non reactive.
d. Mg2+ & Silver are non reactive.
4) Magnesium, Zinc, Copper, Silver
ChemQuandry 1/Building Skills 5
1) Copper, gold, and silver are far from being the most abundant metals on
Earth. Aluminum, iron, and calcium, for example, are all much more plentiful.
Why, then, were copper, gold, and silver among the first metallic elements
discovered? Because they are highly prized in long-lasting, decorative objects and they don't
react with things in nature or other chemicals.
Building Skills 5
Use the table in Figure 16 and the Periodic Table (page 104) to answer the
following questions.
1. a. What trend in metallic reactivity is found from left to right across
a horizontal row (period) of the Periodic Table? (Hint: Compare
the reactivities of sodium, magnesium, and aluminum.) The reactivity of the elements decreases as it moves from left to right on the periodic table.
b. In which part of the Periodic Table are the most-reactive metals
found? Alkali metal
c. Which part of the Periodic Table contains the least-reactive
metals? right side of Transition Metals
2. a. Will iron (Fe) metal react with a solution of lead(II) nitrate,
Pb(NO3)2? Yes
b. Will platinum (Pt) metal react with a lead(II) nitrate solution? Yes
c. Explain your answers to Questions 2a and 2b.
If the solution is a higher has a reactivity than the metal then nothing will happen but if the metal has a higher reactivity than the solution its going to react.
3. Use specific examples from the activity series in your answers to
these two questions:
a. Are least-reactive metals also the cheapest metals? No
b. If not, what other factor(s) might influence the market value of a
metal? They are long lasting and they don’t react with oxygen.
supply and demand
MODELING MATTER
1. Construct a similar electron-dot expression
for the change that occurred in Laboratory
Activity B.4 when each of these events
took place:
a. An atom of zinc, Zn, was converted to a
Zn2 ion. (Hint: Zn has two readily
removable electrons.) Zn: --> Zn2+ + 2e- oxidation
b. A silver ion, Ag+ was converted to a
metallic silver atom, Ag(s). Ag+ + e- -----> Ag. reduction
2. Apply the definitions of oxidation and
reduction to your two equations in Question 1.
3. a. Which reactant (Cu or Ag) is oxidized? copper
b. Which is reduced? Ag+
4. Why are two Ag+ ions needed for each Cu(s)
atom that reacts? Because copper loses two electrons each and the copper atoms are oxidized,so the two electrons are then replaced by the two Ag+ ions.
5. a. Given that definition and explanation, what must be the reducing agent in the reaction between Cu(s) and Ag+ ions? Copper
b. How would you define a reducing agent? The atoms in the reaction loses electrons.
6. Draw an electron-dot representation of this
reaction. Zn2+(s) + Cu(aq) ----> Zn2+ (aq) + Cu(s)
7.Which is the oxidized? a.Cu2+ (aq)
b. Which is the reducing? Zinc
8. Cu2+ (aq) is the oxidizing agent and the zinc is the reducing agent.
9. You could tell by the more reactive element. The most reactive element would be the oxidizing agent and the less reactive one would be the reducing agent.
10.a.The oxidized isZn2+(aq) b.The reduced is Mg(s) c.The oxidizing agent is Zn2+(aq) d.The reducing agent is Mg(s)
RETRIEVING COPPER LAB
Observations
•the black copper turned copper color again
HCL turned yellow
-The zinc reacted right away when it was put in the HCL
- bubbled;fizzed
Questions
1.
In Laboratory Activity B.2 not all of the original copper powder
reacted when you heated it in air.
a. Why do you think the reaction was incomplete? pentine
b. How would you revise the procedure so that more copper(II) oxide could form? Heat it more. Clean them with sandpaper or steel wool.(damage the surface)
2.
a. In Laboratory Activity B.2 what mass of the original copper powder
sample reacted when you heated it? (Hint: Use the
original mass of copper used in Laboratory Activity B.2 and the
mass of copper residue found in Step 8 to calculate this.) .3g of copper powder
b. What percent of the total copper-powder sample reacted? 30%
3.
In the reaction between copper(II) chloride (CuCl2) solution and
zinc metal, each Cu2 ion gained two electrons to form an atom of
copper metal. Each zinc metal atom lost two electrons to form a Zn2 ion.
a. Write a chemical equation that represents this process. (To review how, turn to pages 122–123.) Zn(s) + Cu2+(aq) ---> Zn2+ (aq) + Cu(s)
b. Based on the equation you wrote in Question 3a, identify
i. the species that was oxidized. Zinc
ii. the species that was reduced. copper
iii. the reducing agent. copper
iv. the oxidizing agent. Zinc
4.
Adding HCl to CuO resulted in the formation of a blue solution. Thiscolor is due to the presence of Cu2(aq) ions. Consult your observations in answering these questions:
a. Describe what happened to the solution color after you added zinc in Step 9. The color got brighter and clearer.
b. What caused the changes you observed in the solution? the zinc ions went into the solution.
c. How can the color of the solution be used to indicate when the
zinc metal has removed the Cu2 ions in solution? If the solution has changed from the blue color to the light clear blueish color then you know the zinc metal has been removed.
5. To recover Cu metal from the CuCl2 solution, you had to use other resources.
a. What resources were “used up” in this process?Zinc and HCL
b. Where did each of them go?
READING QUESTIONNAIRE
1.Describe the main differences between renewable and nonrenewable resources and provide an example of each. Renewable resources can be replenished and a nonrewable resource can't be replenished. An example for a renewable resource air and an example for nonrenewable resource is natural gas.
2. a) If atoms are always conserved why do some people say that a resource may be “running out”?
b) Can a resource actually “run out”?
3.) What are the requirements for minimum profitability levels for a metal in an ore? As low as 1% for copper or 0.001% for gold to as high as 30% of aluminum.
4.) Identify and explain the two strategies for avoiding the depletion of metal ores.
Slowing down the rate of the use of resources.
Replace a resource by finding substitute materials with similar properties.
5.) Can recycling also create environmental problems? If so, explain how this can happen. Yes because aluminum scaps may contain up to 1% of magnesium and to properly remove the magnesium they would have to use chlorine gas which can lead to air pollution.
6.) How much trash does the average person produce per day? 4lbs a day.
7.) Identify two ways that consumer products can become waste. telephones and yesterday's newpaper.
8.)Describe a way of dealing with recyclable waste that might be profitable good for energy use. combustion for energy. ( waste-to-energy)
9.)What are the three options for the final step in the life cycle of a material? Recycle,Landfills, and combustion for energy.
10.) Which waste category has the greatest weight before recycling? What is the weight of this waste produced? Paper, 83.8 million tons.
11.) Using Figure 21 on page147 identify which waste category has the least weight before recycling? What is the weight of this waste? Wood, 11.6 million tons
12.)Calculate the difference between the waste produced from your answer to question 11 and the amount of waste produced after recycling. Remember these values are in millions of tons, so make sure that you calculate correctly and label with the correct units of measure. (1 ton = 2000 lbs) .6million tons
13.)If we compare the Total Generation of Waste (before recycling) to the Total Discards of Waste (after recycling), what percentage of waste is actually thrown away? What percentage of the Total Generation of Waste is actually recycled? Show your calculations below using the correct units of measure and labels. 72% of actual waste is thrown away. 28% total generation of waste is actually recycled
14.) Draw the diagram in Figure 22, on page 148, in the space below. Compare this to Figure 20 on page 146. Match and Label the location of the steps in figure 20 to your diagram by connecting them with lines/arrows around the outside. will show you in class
BUILDING SKILLS 11
1)
STRIKING IT RICH LAB
Observations
-when the pennies were dropped into the Zn and ZnCl2 solution it then dark grey then when dropped into the water it turned silver like a nickel.
- the pennies were put into the flame then dropped into water the pennies started to take on a gold color.
heated in burner flame
1) a. The untreated penny is a copper/bronze color,look like a ordinary penny. The penny treated with the Zn and ZnCl2 has a silver coating and the penny with Zn and ZnCl2 and heated in the burner flame has a gold coating.
b. Yes the penny treated with Zn and ZnCl2 is composed of Copper and Zinc and the penny treated with Zn and ZnCl2 and the burner is composed of Zinc and Copper. (True, but what does the penny "look" like? Does it appear to be "gold" or "silver"?) -1
2) Their claim would be incorrect because the penny is made of copper and it just has a coating on of zinc on it. (Prove it. What does the Law of Conservation of Matter say?) -2
3) Pipes and bridges (Pipes maybe but bridges? This type of process is more for coating common materials like jewelry or something smaller.) -1
4) a. The copper atoms went into the solution.(No the copper atoms stayed right where they were, in the penny.) -2
b. Yes. The same procedure from the Retrieving copper activity would have to be done in order to convert the pennies back to its copper state. (You could do that. Good answer.)
BUILDING SKILLS 12
1) Pluming(pipes) - Lead
Electrical wiring- silver
Pot and pans- iron
shell casing- silver
2) magnesium,potassium,lithium,
3) shell casings and electrical wiring because its would last longer.
SECTION 3.A
HYDROCARBON BOILING POINTS
1) A. Its organized in alphabetical order.
B.Yes because it can help people remember the names and the boiling points.
2) A. Lowest to highest boiling point.
B.
3) Butane,Propane,Ethane,Methane
4) Petane
5) The intermolecular forces in Decane are more active than those in Butane.
SEPARATION BY DISTILLATION LAB QUESTIONS (30/42)
2) A. 86degrees C; 95 degrees C
3) Distillation 1 was Acetone and Distillation2 was Propanol. (D-1 = propanol, D-2 = water -2)
4) Didn't get information. (-2)
5) Distillation 2 because it reacted with iodine better than distillation 1.
6) By looking at the appearance or test samples of the solution against other substances. (explain? -1)
7) Cyclohexane and water because it is a long and drawn out process that takes to much energy. (What about propanol? Isn't the boiling point closest to cyclohexane? -1)
8) ? (-6)
BUILDING SKILLS 3
1) The more the carbon-chain branches increases the higher the boiling point because there is more energy needed to move the atoms around.
a. 98.4 degreesC
b. 92.0 degreesC
c. 79.2 degreesC
3)
a. The figure would have a lower BP than the single chain and the one branch chain. It would also have a higher BP than the three branch.
b. Higher
4.) The parent chain determines the boiling point, so the longer the parent chain the boiling point.The straighter the chain the higher the BP and the more it branches out the lower the BP will be.